Stoichiometric Relationships

Stoichiometry - the quantitative relationships between reactants and products in chemical reactions, helps in understanding the composition of substances and predicting the outcomes of reactions.

Balancing Chemical Equations

• Balancing equations using coefficients ensures that the law of conservation of mass is obeyed.

• Identifying the stoichiometry of a reaction helps in determining the relative amounts of reactants and products.

Combustion Equations: burning organic compounds - CH4 + 2O2 = CO2 + 2H2O

Ionic Equations: aqueous solutions break apart compounds into ions

Ideal Gases: Ideal gases are hypothetical gases whose particles have negligible volume and no attractive forces. They follow the ideal gas law, PV = nRT, where P is pressure, V is volume, n is moles of gas, R is the gas constant, and T is temperature.

Mole Concept

• Understanding Avogadro's number (6.022 x 10^23) helps in converting between moles and particles.

• Calculating molar mass allows us to convert between grams and moles of a substance.

Empirical Formula:

Stoichiometric Calculations

• Applying mole ratios in stoichiometric calculations helps in determining the amounts of reactants consumed and products produced.

• Recognizing the limiting reactant is crucial for predicting the maximum amount of product that can be formed.

Percentage Yield

• Calculating the percentage yield involves comparing the actual yield of a reaction to the theoretical yield.

• Factors such as impurities, side reactions, and incomplete reactions can affect the efficiency of a reaction.

Sub-branches:

• Mole Concept:

  • Avogadro's number represents the number of particles in one mole of a substance.

  • Molar mass is the mass of one mole of a substance and is expressed in grams per mole.

• Balancing Chemical Equations:

  • Chemical equations are balanced based on whole number ratios of moles.

  • The law of conservation of mass states that mass is conserved in a chemical reaction.

• Stoichiometric Calculations:

  • Conversion factors are used to convert between different units of measurement.

  • Identifying the excess reactant helps in determining the limiting reactant and the maximum amount of product that can be obtained.

• Percentage Yield:

  • Calculating the efficiency of a reaction provides insight into the success of the reaction.